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The nucleus has a width on the order of 10^(-15) meters, while an electron is (on average) a distance of 10^(-10) meters from the nucleus. If you were to magnify the nucleus to the size of a baseball, the electrons would be orbiting at a distance of around 1000 meters. That is, there are about 50,000-100,000 nucleus diameters to the electron's average radius.
No. The greater distance from the nucleus the more energy an electron has.
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Because if the radius is big, then the large distance affects the strenght of the electron with the nucleus. This also increases reactivity in non metals since it will be easier to take away the electron :)
The energy possessed by an electron at a set of distance from the nucleus.
The nucleus has a width on the order of 10^(-15) meters, while an electron is (on average) a distance of 10^(-10) meters from the nucleus. If you were to magnify the nucleus to the size of a baseball, the electrons would be orbiting at a distance of around 1000 meters. That is, there are about 50,000-100,000 nucleus diameters to the electron's average radius.
Shell
It would not depend on the direction with respect to the nucleus. The direction of the electron has no effect on the distance of the electron from the nucleus.
An electron in a 2s orbital is on average closer to the nucleus.
The atomic radius is the distance from the nucleus of an atom to the outermost orbital of electron.
No. The greater distance from the nucleus the more energy an electron has.
Although there exists a non-zero probability for an electron to be within the nucleus, the greatest probability is for them to be found somewhere outside there. The average (more precisely, the expectation value of the) distance between an electron and the nucleus is represented by the different periods of the periodic table. With an increasing period number comes an increasing average distance.
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The path of a given electron's orbit around a nucleus, marked by a constant distance from the nucleus.